1. Review for test

2. * What are the 3 theories of acids and bases? * Lavoisier * Arrhenius * Br Ø nsted-Lowry * Lewis

3. * What are conjugate pairs? * They differ by one proton or a H+.

4. * What are the general properties of acids and bases? * React differently with indicators. * Acids react with metals, bases, carbonates. * They can be strong or weak. * Low pH or high pH.

5. * How do we use pH and properties of water in calculations? * pH = -log[H+] pOH = -log[OH-] * Kw = [H+] [OH-] * Kw has different values depending on temperature. * The concentrations are inversely related. * What is the pH of blood that has 4.60 x 10 -8 H+ concentration at 25º C? (Kw = 1x10 -14 )

6. * How do pH and pOH relate? * pH + pOH = 14.00 at 25º C. * pH and pOH can be found from concentrations of strong acids and bases * Ka is acid dissociation constant. * How is it different for strong and weak?

7. * What is the Ka of.0100 M ethanoic acid with a pH of 3.4? * pH = -log [H+] *.01 – 4 x10 -4 * Acid dissociation equation. * How about.75 M with a Ka of 1.8 x 10 -5 has what pH?

8. * What are pKa and pKb? * These are negative logs of base 10 of Ka and Kb. * This gives positive values with no units. * Ka and pKa have inverse relationship (b also). * A change in one unit of pKa represents 10 the change in Ka (b also). * They are all still temperature related.

9. * What is the relationship between Ka and Kb and pKa and pKb? * Ka x Kb = [H+] [OH-] = Kw * pKa + pKb = pKw * pKa + pKb = 14 at 25C

10. * What are buffer solutions? * Buffers resist change in pH (pOH) with addition of small amounts of acid or base. * Acidic buffers are a weak acid and salt of weak acid and strong base. * Basic buffers are a weak base and salt of weak base with a strong acid. * They act on LeChatlier’s principle.

11. * How do we find the pH of a buffer solution? * Henderson-Hasselbalch equation * pH = pKa + log [salt]/[acid] * pOH = pKb + log [salt]/[base] * What is the pH of 25 mL of ethanoic acid and sodium ethanote with a Ka of 1.8 x 10 -5 ?

12. * What is salt hydrolysis? * All acid base reactions create salts (cation from base and anion from acid). * If there is a weak acid, the anion is a strong enough that can it hydrolyse water releasing OH. * If there is a weak base and the cation is a nonmetal, it is able to hydrolyse water relasing H. * If the metal is small with a decent charge density, it acts like a ligand complex and takes OH out of the solution. (Be, Al, Fe)

13. * What is titration? * It is a controlled acid base neutralization reaction trying to find the equivalence point. * This is used to find the concentration of an unknown with a known amount of a known concentration.

14. * What are titration curves?

15. *W*W hat are indicators? *T*T hey are sensitive to changes in pH. *T*T hey change colors at specific pH’s. *C*C hange color when pKa = pH. *T*T his is the end point. *U*U sed to find equivalence points in titrations.